Which of the following statements is incorrect?

Options

A. A sigma bond has no free rotation around its axis.
B. Two p orbitals always overlap laterally.
C. There can be more than one sigma bond between two atoms.
D. All of these

Explanation

To determine which of the following statements is incorrect, let's analyze each statement step by step:

1. **Statement A**: "A sigma bond has no free rotation around its axis."
- **Analysis**: This statement is incorrect. A sigma bond is formed by the axial (end-to-end) overlap of orbitals, which allows for free rotation around the bond axis. In contrast, pi bonds, which are formed by lateral (sideways) overlap, do not allow for rotation without breaking the bond. Therefore, this statement is false.

2. **Statement B**: "2p orbitals always overlap laterally."
- **Analysis**: This statement is also incorrect. While p orbitals can overlap laterally (sideways), they can also overlap linearly (end-to-end). For example, two p orbitals can align along the same axis, allowing for linear overlap. Thus, stating that 2p orbitals always overlap laterally is misleading and incorrect.

3. **Statement C**: "There can be more than one sigma bond between two atoms."
- **Analysis**: This statement is incorrect as well. According to the principles of chemical bonding, only one sigma bond can exist between two atoms. Additional bonds between the same two atoms must be pi bonds. For instance, in a triple bond (like in N2), there is one sigma bond and two pi bonds. Therefore, this statement is false.

4. **Conclusion**: Since all three statements (A, B, and C) are incorrect, the correct answer is that all statements are incorrect.

**Final Answer**: All statements are incorrect.

---